Question

The following reaction occurs in aqueous solution: NH4 + (aq) + NO2 - → N2 (g) + 2H2O (l) The data below is obtained at 25°C. [NH4 +] (M) [NO2 -] (M) Initial rate (M/s) 0.0100 0.200 3.2 × 10-3 0.0200 0.200 6.4 × 10-3 The order of the reaction in NH4 + is __________.

Answer 1

Answer: The order with respect to
`NH_4^+` is 1.

Step-by-step explanation:

Rate law says that rate of a reaction is directly proportional to the concentration of the reactants each raised to a stoichiometric coefficient determined experimentally called as order.

`NH_4^++NO_2^-\rightarrow N_2+2H_2O`

`Rate=k[NH_4^+]^x[NO_2^-]^y`

k= rate constant

x = order with respect to
`NH_4^+`

y = order with respect to A
`NO_2^-`

n = x+y = Total order

From trial 1:
`3.2* 10^(-3)=k[0.0100]^x[0.200]^y` (1)

From trial 2:
`6.4* 10^(-3)=k[0.0200]^x[0.200]^y` (2)

Dividing 2 by 1 :
`(6.4* 10^(-3))/(3.2* 10^(-3))=(k[0.0100]^x[0.2000]^y)/(k[0.0200]^x[0.200]^y)`

`2=2^x,2^1=2^x` therefore x= 1

Thus order with respect to
`NH_4^+` is 1.